Define Dipolemoment. Write its applications.

Explanation

Dipolemoment is the product of the magnitude of the charge and the distance between the centres of positive and negative charges. It is designated by `mu`.
Dipolemoment `(mu)` = Charge(Q) `times` distance(r) between the charges.
Units of dipolemoment are Debye units (D)
Applications :
1) Dipolemoment is useful in calculating the percent ionic character of polar covalent bonds.
% ionic character = `(mu_(obs))/(mu_(ionic))times100`
2) Dippolemoment is useful in predicting the shapes of molecules. e.g.,
i) In the case of `Ax_(2)` type molecule if dipolemoment is zero they have linear structure but if they have some dippolemoment they are angular.
ii) `AX_(3)` type molecules with dipolemoment zero are planar triangular in shape but if they have some dipolemoment they have pyramidal shape.
iii) `AX_(4)` type molecules with dipolemoment zero have symmetric tetrahedral structure but if they have some dipolemoment they have distorted tetrahedral shape.
iv) In geometrical isomers trans isomers have zero dipolemoment. While cis isomers have some dipole-moment.
3. It is useful to predict the polarity of molecule.
i) Molecular with dipolemoment is greatrer than zero are polar.
ii) Molecular with dipolemoment is equal to zero are non polar.